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1. Define oxidation numberm oxidation, reduction, reducing agent and oxidizing agent. 2. What is oxidized and what is reduced in the following reaction: N2 + 202 → 2NO2

1. Define oxidation numberm oxidation, reduction, reducing agent and oxidizing agent. 2. What is oxidized and what is reduced in the following reaction: N2 + 202 → 2NO2

Chemistry
Chemistry
9th Edition
ISBN:9781133611097
Author:Steven S. Zumdahl
Publisher:Steven S. Zumdahl
Chapter4: Types Of Chemical Reactions And Solution Stoichiometry
Section: Chapter Questions
Problem 10RQ
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SCH4U1 Assignment 5 1. Define oxidation numberm oxidation, reduction, reducing agent and oxidizing agent. 2. What is oxidized and what is reduced in the following reaction: N2 + 202→ 2NO2 3. Determine the oxidation number of each element in the following substances: a ) H2SO4 d ) KMNO4 b) Ca3(PO4)2 e ) H3ASO4 с) Clz f) CaSnO3 4. Balance the following equations (use the oxidation number method): a) MnO4¯ + Fe b) HNO3 + H;S c) Cr2O,²- + ci~ d) Cr(OH)3(s) + ClO;'(aq) Mn?* + Fe* (acidic solution) NO + S + Cl2 (acidic solution) CrO2 (aq) + Cl'(aq) (basic solution) 5. Iodine normally has oxidation numbers of -1 and 0. Could I2 serve as a reducing agent? Explain why or why not. 6. Describe what happens when chlorine in water is mixed with bromide ions and cyclohexane (a non-polar solvent). Explain why this happens. 7. Should chlorine gas be passed through copper tubing? Explain your answer using Eº values. 8. Balance the following equations using the half-reaction method. а) Ва (s) + CI, b) Zn (s) + S0,- + H* c) MnO4 + NO, + H2O d)r + NO,¯ + H' Ba* + CI H,SO3 (g) + Zn²* + H,O Mn* + NO, + H* h + NO2 + H2O 9. For each set of reactants, write a redox equation for the reaction that may occur. Calculate the E°cell values and determine if the reaction is spontaneous. a) Mg(s) + A1³* d) Sn(s) + H* b) Hg** + Ag(s) e) H2(g) + C12(g) c) CI + ½(s) ) Cu(s) + I 10. Name two substances which oxidize Ag to Ag*. 11. Draw the following galvanic (voltaic) cells (salt bridge design) and label the following: i) anode and cathode ii) oxidation and reduction half reaction iii) direction of electron, cation and anion movement iv) net reaction v) calculate the E cll a) Co«) |Co(NO3)2 (aq) || Zn(NO3)2 (aq) | Zn (s) (standard conditions) b) Au(s) |Au(NO;); (aq) || H2(g), HCI (aq) | Pt (s) (hydrogen standard cell) c) Sn(s) |Sn{NO3))2 (1.00 M) || Zn(NO)2 (0.0100 M) | Zn(s)
Transcribed Image Text:SCH4U1 Assignment 5 1. Define oxidation numberm oxidation, reduction, reducing agent and oxidizing agent. 2. What is oxidized and what is reduced in the following reaction: N2 + 202→ 2NO2 3. Determine the oxidation number of each element in the following substances: a ) H2SO4 d ) KMNO4 b) Ca3(PO4)2 e ) H3ASO4 с) Clz f) CaSnO3 4. Balance the following equations (use the oxidation number method): a) MnO4¯ + Fe b) HNO3 + H;S c) Cr2O,²- + ci~ d) Cr(OH)3(s) + ClO;'(aq) Mn?* + Fe* (acidic solution) NO + S + Cl2 (acidic solution) CrO2 (aq) + Cl'(aq) (basic solution) 5. Iodine normally has oxidation numbers of -1 and 0. Could I2 serve as a reducing agent? Explain why or why not. 6. Describe what happens when chlorine in water is mixed with bromide ions and cyclohexane (a non-polar solvent). Explain why this happens. 7. Should chlorine gas be passed through copper tubing? Explain your answer using Eº values. 8. Balance the following equations using the half-reaction method. а) Ва (s) + CI, b) Zn (s) + S0,- + H* c) MnO4 + NO, + H2O d)r + NO,¯ + H' Ba* + CI H,SO3 (g) + Zn²* + H,O Mn* + NO, + H* h + NO2 + H2O 9. For each set of reactants, write a redox equation for the reaction that may occur. Calculate the E°cell values and determine if the reaction is spontaneous. a) Mg(s) + A1³* d) Sn(s) + H* b) Hg** + Ag(s) e) H2(g) + C12(g) c) CI + ½(s) ) Cu(s) + I 10. Name two substances which oxidize Ag to Ag*. 11. Draw the following galvanic (voltaic) cells (salt bridge design) and label the following: i) anode and cathode ii) oxidation and reduction half reaction iii) direction of electron, cation and anion movement iv) net reaction v) calculate the E cll a) Co«) |Co(NO3)2 (aq) || Zn(NO3)2 (aq) | Zn (s) (standard conditions) b) Au(s) |Au(NO;); (aq) || H2(g), HCI (aq) | Pt (s) (hydrogen standard cell) c) Sn(s) |Sn{NO3))2 (1.00 M) || Zn(NO)2 (0.0100 M) | Zn(s)
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